Rates of Reactions

Introductory Activity:

Monitoring the mass of the coca-cola over time:

Time (s)	Mass (g)
0	86.730
10	86.718
20	86.710
30	86.702
40	86.697
50	86.692
60	86.686
70	86.685
80	86.680
90	86.679
100	86.676
110	86.673
120	86.671
130	86.667
140	86.664
150	86.661
160	86.660
170	86.658
180	86.656
190	86.651
200	86.650
210	86.648

Put all of this data into excel. Create a new column and determine the total mass of CO2 formed for each time value. Convert mass of CO2 into moles of CO2. Put the number of moles of CO2 into the new column.

a) Plot Moles of CO2 produced against time.
b) Create another column next to the moles of CO2 produced for moles of H2CO3 decomposed.
c) Plot Moles of H2CO3 decomposed against tme.
b) Calculate the average rate of CO2 production between t= and t=
c) Calculate the instantaneous rate of CO2 production at t=0
d) Calculate the instantaneous rate of CO2 production at t=
d) Write out the balanced chemical reaction that is occuring
e) For the same times as selected for questions b), c), and d), determine the instantaneous rate of decomposition of H2CO3.

Graphs: